First Semester Final - Review Questions
... 37. Describe the different amounts and kinds of damage in matter produced by the different penetrations of each type of radioactive decay. 38. How does the energy release in a nuclear reaction compare to the energy release in a chemical reaction. Investigation and Experimentation 39. What is the pur ...
... 37. Describe the different amounts and kinds of damage in matter produced by the different penetrations of each type of radioactive decay. 38. How does the energy release in a nuclear reaction compare to the energy release in a chemical reaction. Investigation and Experimentation 39. What is the pur ...
The geometry of a molecule is determined only by location of the
... Exceptions to the rule includes all elements that have d levels close in energy. However, much of their chemistry can still be explained by the octet rule. ...
... Exceptions to the rule includes all elements that have d levels close in energy. However, much of their chemistry can still be explained by the octet rule. ...
Slide 1 - Effingham County Schools
... pairs that will be arranged at an angle of 180 degrees. •We need a pair of atomic orbitals oriented in opposite directions (sp orbitals). ...
... pairs that will be arranged at an angle of 180 degrees. •We need a pair of atomic orbitals oriented in opposite directions (sp orbitals). ...
Chemical Bonding
... A bonding molecular orbital places a high electron charge density between the two nuclei. This reduces the repulsions between the positively charged nuclei, lowering the energy and increasing the stability of the molecule. An anti-bonding molecular orbital places a low electron charge density betwee ...
... A bonding molecular orbital places a high electron charge density between the two nuclei. This reduces the repulsions between the positively charged nuclei, lowering the energy and increasing the stability of the molecule. An anti-bonding molecular orbital places a low electron charge density betwee ...
Chapter 7 Covalent Bonds and Molecular Architecture
... Octet rule: Main group elements tend to undergo reactions that leaves them with either 2 or 8 electrons in their outer or valence shell achieved by sharing electrons. Exceptions to the rule includes all elements that have d levels close in energy. However, much of their chemistry can still be expla ...
... Octet rule: Main group elements tend to undergo reactions that leaves them with either 2 or 8 electrons in their outer or valence shell achieved by sharing electrons. Exceptions to the rule includes all elements that have d levels close in energy. However, much of their chemistry can still be expla ...
MOLECULAR ORBITAL AND VALENCE BOND THEORY EXPLAINED
... An antibonding molecular orbital (designated with an *) occurs when the electron density of the orbital is concentrated in regions of space outside the area between the atomic nuclei. Electrons in antibonding molecular orbitals do not stabilize covalent bonds because the electrons are not position ...
... An antibonding molecular orbital (designated with an *) occurs when the electron density of the orbital is concentrated in regions of space outside the area between the atomic nuclei. Electrons in antibonding molecular orbitals do not stabilize covalent bonds because the electrons are not position ...
molecular orbital and valence bond theory explained (hopefully)
... A bonding molecular orbital occurs when the electron density of the orbital is concentrated between the atomic nuclei. Electrons in bonding molecular orbitals stabilize covalent bonds because they serve to offset the repulsive forces of the positively-charged atomic nuclei. Both nuclei are attr ...
... A bonding molecular orbital occurs when the electron density of the orbital is concentrated between the atomic nuclei. Electrons in bonding molecular orbitals stabilize covalent bonds because they serve to offset the repulsive forces of the positively-charged atomic nuclei. Both nuclei are attr ...
Chemistry I Honors
... b.On the basis of the Lewis structures drawn in part (a), answer the following questions about the particular species indicated. i. What is the Cl-Ge-Cl bond angle in GeCl4? ...
... b.On the basis of the Lewis structures drawn in part (a), answer the following questions about the particular species indicated. i. What is the Cl-Ge-Cl bond angle in GeCl4? ...
Bonding Conceptually easier to view bonding if one considers
... Electron density is not symmetric about the internuclear axis ...
... Electron density is not symmetric about the internuclear axis ...
Hybrid Orbitals
... We think of covalent bonds forming through the sharing of electrons by adjacent atoms. In such an approach this can only occur when ...
... We think of covalent bonds forming through the sharing of electrons by adjacent atoms. In such an approach this can only occur when ...
Text Related to Segment 7.01 ©2002 Claude E. Wintner To make a
... which determine how atoms are held in association with one another. Only then will we be able to proceed to the study of "grammar" — the rules governing the transformations of molecules, or reactions, that are the specific domain of the chemist. When two hydrogen atoms are brought together from "inf ...
... which determine how atoms are held in association with one another. Only then will we be able to proceed to the study of "grammar" — the rules governing the transformations of molecules, or reactions, that are the specific domain of the chemist. When two hydrogen atoms are brought together from "inf ...
Key Concepts PowerPoint
... The following ball-and-stick molecular model is a representation of thalidomide, a drug that causes birth defects when taken by expectant mothers but is valuable for its use against leprosy. The lines indicate only the connections between atoms, not whether the bonds are single, double, or triple (r ...
... The following ball-and-stick molecular model is a representation of thalidomide, a drug that causes birth defects when taken by expectant mothers but is valuable for its use against leprosy. The lines indicate only the connections between atoms, not whether the bonds are single, double, or triple (r ...
Quantum Mechanics Quantum Mechanics Quantum Numbers
... Exceptions to the rule A d subshell that is half-filled or full (ie 5 or 10 electrons) is more stable than the s subshell of the next shell. This is because it takes less energy to maintain an electron in a half-filled d subshell than a filled s subshell. For instance, copper (atomic number 29) has ...
... Exceptions to the rule A d subshell that is half-filled or full (ie 5 or 10 electrons) is more stable than the s subshell of the next shell. This is because it takes less energy to maintain an electron in a half-filled d subshell than a filled s subshell. For instance, copper (atomic number 29) has ...
Electron and Molecular Geometries
... 3) Allow for any ion charge. For example, if the ion has a 1- charge, add one more electron. For a 1+ charge, deduct an electron. 4) Divide by 2 to find the total number of electron pairs around the central atom. 5) Work out how many of these are bonding pairs, and how many are lone pairs. You know ...
... 3) Allow for any ion charge. For example, if the ion has a 1- charge, add one more electron. For a 1+ charge, deduct an electron. 4) Divide by 2 to find the total number of electron pairs around the central atom. 5) Work out how many of these are bonding pairs, and how many are lone pairs. You know ...
Fehling`s Test / Benedict`s Test
... Thus, there are only three bond pairs around the central boron atom, which are arranged in a trigonal planar geometry with bond angles of 1200 so as to minimize the repulsion (see [2]). While in the case of NF3, 26 valence electrons give rise to three bond pairs and one lone pair on the central N at ...
... Thus, there are only three bond pairs around the central boron atom, which are arranged in a trigonal planar geometry with bond angles of 1200 so as to minimize the repulsion (see [2]). While in the case of NF3, 26 valence electrons give rise to three bond pairs and one lone pair on the central N at ...
CHM134 General Chemistry I Semester Review – Dr. Steel This list
... 21. If n = 3, what are the allowed quantum numbers for l? 22. What element has the ground state electron configuration: [Ar]4s13d5? 23. What element has the ground state electron configuration: [Kr]5s2? 24. What is the maximum number of electrons permitted in a d sublevel? 25. Green light has a wave ...
... 21. If n = 3, what are the allowed quantum numbers for l? 22. What element has the ground state electron configuration: [Ar]4s13d5? 23. What element has the ground state electron configuration: [Kr]5s2? 24. What is the maximum number of electrons permitted in a d sublevel? 25. Green light has a wave ...
Chapter 6 Quiz
... ______10. When atoms share electrons, the electrical attraction of an atom for the shared electrons is called the atom's a. electron affinity. b. resonance. c. electronegativity. d. hybridization. ______11. If the atoms that share electrons have an unequal attraction for the electrons, the bond is c ...
... ______10. When atoms share electrons, the electrical attraction of an atom for the shared electrons is called the atom's a. electron affinity. b. resonance. c. electronegativity. d. hybridization. ______11. If the atoms that share electrons have an unequal attraction for the electrons, the bond is c ...
Masterton and Hurley - Chapter 7
... Covalent Bonding NOT IN NOTES • Recall that electrons in atoms are placed into atomic orbitals according to the Aufbau (fill 1st energy level first), Pauli (2 e-s per orbital), and Hund’s Rules (1 e- in each first within a sublevel) • In this section of the course, we will look at the location of e ...
... Covalent Bonding NOT IN NOTES • Recall that electrons in atoms are placed into atomic orbitals according to the Aufbau (fill 1st energy level first), Pauli (2 e-s per orbital), and Hund’s Rules (1 e- in each first within a sublevel) • In this section of the course, we will look at the location of e ...
Inorganic Pharmaceutical Chemistry Hybrid Orbitals Hybridization
... If your visual imagination will cope, you may be able to see that this ion has no plane of symmetry. If you find this difficult to visualise, the only solution is to make the ion out of a lump of plasticene (or a bit of clay or dough) and three bits of cardboard cut to shape A substance with no plan ...
... If your visual imagination will cope, you may be able to see that this ion has no plane of symmetry. If you find this difficult to visualise, the only solution is to make the ion out of a lump of plasticene (or a bit of clay or dough) and three bits of cardboard cut to shape A substance with no plan ...
First Semester Honors Chemistry Exam Review (2011
... 38. A spherical electron cloud surrounding an atomic nucleus would best represent which orbital (s)? 39. How many orbital shapes are in the first energy level? Second? Third? Fourth? What are they? 40. Both copper (atomic number 29) and chromium (atomic number 24) appear to break the pattern in the ...
... 38. A spherical electron cloud surrounding an atomic nucleus would best represent which orbital (s)? 39. How many orbital shapes are in the first energy level? Second? Third? Fourth? What are they? 40. Both copper (atomic number 29) and chromium (atomic number 24) appear to break the pattern in the ...
Bent's rule
Bent's rule describes and explains the relationship between the isovalent hybridization of central atoms in molecules and the electronegativities of substituents. The rule was stated by Henry Bent as follows: ""Atomic s character concentrates in orbitals directed toward electropositive substituents"".The chemical structure of a molecule is intimately related to its properties and reactivity. Valence bond theory proposes that molecular structures are due to covalent bonds between the atoms and that each bond consists of two overlapping and typically hybridised atomic orbitals. Traditionally, p-block elements in molecules are assumed to hybridise strictly as spn, where n is either 1, 2, or 3. In addition, the hybrid orbitals are all assumed to be equivalent (i.e. the n+1 spn orbitals have the same p character). Results from this approach are usually good, but they can be improved upon by allowing hybridised orbitals with noninteger and unequal p character. Bent's rule provides a qualitative estimate as to how these hybridised orbitals should be constructed. Bent's rule is that in a molecule, a central atom bonded to multiple groups will hybridise so that orbitals with more s character are directed towards electropositive groups, while orbitals with more p character will be directed towards groups that are more electronegative. By removing the assumption that all hybrid orbitals are equivalent spn orbitals, better predictions and explanations of properties such as molecular geometry and bond strength can be obtained.Bent's rule can be generalized to d-block elements as well. The hybridisation of a metal center is arranged so that orbitals with more s character are directed towards ligands that form bonds with more covalent character. Equivalently, orbitals with more d character are directed towards groups that form bonds of greater ionic character.